A student ran the following reaction in the laboratory at 322 K: 2NO(g) + Br2(g) = 2NOB1(g) When she introduced 0.107 moles of NO(g) and 9.86×10² moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 7.65×10² M. Calculate the equilibrium constant, Ke, she obtained for this reaction. K. =

A student ran the following reaction in the laboratory at 322 K: 2NO(g) + Br2(g) = 2NOB1(g) When she introduced 0.107 moles of NO(g) and 9.86×10² moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 7.65×10² M. Calculate the equilibrium constant, Ke, she obtained for this reaction. K. =

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 60QRT

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